I am having so much trouble understanding how to classify reactions as precipitation, acid base, or oxidation reduction. In one example in particular, it reads Iron II oxide reacts with oxygen and water to yield Iron III hydroxide. I wrote out the equation as: FeO(aq)+O2(g)+H2O(l)=FeOH3(s). I was thinking it was oxidation reduction but it produces a solid so that got me thinking its a precipitation reaction! Which ultimately got me thinking I really don't understand how to classify them. Also, it's impossible to balance this equation. I've double checked my symbols and I don't know what's going on.
1. It won't balance because you don't have the right formula down. The left side is ok but iron(III) hydroxide is Fe(OH)3,
2. It is a pptn reaction because aq/g/l on the left goes to a solid on the right. However, it ALSO is a redox reaction. Fe on the left is +2 and on the right is +3 so Fe is oxidized. O2 on the left is zero and on the right is -2; therefore, O2 is reduced. Note that the O in FeO is -2 on the left and -2 on the right; it is not involved in the redox part. Having said all of that, I suspect you are to report this as a redox reaction. Although a ppt forms it isn't a typical pptn type reaction.
Oh my goodness! Thank you so much for pointing that out. Two little brackets - and it balanced just fine. Thank you also for explaining that this can be seen both ways, technically. It gives me a little more confidence.
While eating supper it occurred to me that something was amiss about that problem. How do you get an aqueous solution of FeO. FeO is a solid and very little of it will dissolve. This may be one of a series of reactions for the formation of rust. Anyway, I wonder if that should have been FeO(s) and if so then a solid going to a solid will not be a pptn reaction even though the solids are different.
Thank you for that. Chemistry is the most challenging class for me and I am the one that assigned it (aq) because all that still confuses me too. In the original problems, we were just given the words and we need to write the chemical formulas. I get confused about when to use (aq) (s) (l) and (g), well actually (g) is the easy one. Initially I was just using the solubility rules to determine if something would be a solid but then found that's not always correct because when I look back at my instructor's powerpoint, I find she uses (aq) for things that I would call (s) so I find I'm sometimes just giving it my best guess.
Generally you will be right doing it that way. If the material is soluble and you have a liquid solution (such as HCl, H2SO4, HNO3, etc are all in aq solution) so the solubility rules work very well. Yes, gases are easy. If you're mixing solutions that makes it easy, too.
Understanding how to classify chemical reactions is essential in chemistry. Let's break down the reaction you mentioned to help you understand how to classify it.
The given reaction is: Iron II oxide reacts with oxygen and water to yield Iron III hydroxide.
First, let's write the correct chemical equation:
FeO(s) + O2(g) + H2O(l) → Fe(OH)3(s)
To classify a reaction, we need to identify the types of reactions that potentially take place. Here are the three categories you mentioned:
1. Precipitation reaction: In a precipitation reaction, an insoluble solid (called a precipitate) is formed when two aqueous solutions react.
2. Acid-base reaction: In an acid-base reaction, an acid and a base react to form water and a salt.
3. Oxidation-reduction (redox) reaction: In a redox reaction, the oxidation states of some elements change due to the transfer of electrons.
Now, let's analyze the given reaction:
FeO(s) + O2(g) + H2O(l) → Fe(OH)3(s)
In this reaction, the solid FeO is reacting with O2(g) and H2O(l) to produce the solid Fe(OH)3.
To classify this reaction, we need to consider the nature of the reactants and products.
1. Precipitation reaction: In this case, solid Fe(OH)3 is formed, suggesting it is a precipitate. Therefore, we can classify this reaction as a precipitation reaction.
2. Acid-base reaction: Since there are no acid or base compounds involved in the reaction, we can exclude acid-base reaction as a classification for this particular reaction.
3. Oxidation-reduction reaction: To determine if an oxidation-reduction reaction is taking place, we need to analyze the oxidation states of the elements involved. In this reaction, the oxidation states of Fe and O do not change. Therefore, it is not an oxidation-reduction reaction.
In summary, based on the formation of a solid precipitate, we can classify the given reaction as a precipitation reaction. It is important to note that some reactions can fall into multiple categories, but in this case, precipitation is the primary classification.
Regarding balancing the equation, you are correct that the equation you provided is not balanced. In a balanced equation, the number of atoms on both sides of the equation should be equal. To balance the equation, you need to adjust the coefficients in front of each compound until the atoms are balanced on both sides.